Home
Class 12
CHEMISTRY
A 0.25 M solution of pyridinium chloride...

A `0.25 M` solution of pyridinium chloride `C_(5)H_(5)NH^(+)Cl^(-)` was found to have a `pH` of `2.75` What is `K_(b)` for pyridine, `C_(5)H_(5)N`?

Text Solution

Verified by Experts

The correct Answer is:
`k_(b)=6.25 xx 10^(-10)`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRUIM

    MOTION|Exercise Exercise -4 (Level -1)|19 Videos

  • IONIC EQUILIBRUIM

    MOTION|Exercise Exercise -4 (Level -II)|14 Videos

  • IONIC EQUILIBRUIM

    MOTION|Exercise Exercise -2 (Level -II)|31 Videos

  • HYDROCARBON

    MOTION|Exercise Exercise - 4 (Level-II)|15 Videos

  • ISOMERISM

    MOTION|Exercise Exercise 4|26 Videos

Similar Questions

Explore conceptually related problems

A 0.25 M solution of pyridinium chloride, C_(5)H_(5)NH^(+)Cl^(-) , was found to have a pH of 2.89 . What is the K_(b) for pyridine, C_(5)H_(5)N ?

A 0.25M solution of pyridinium chloride (C_(5)H_(5)overset(o+)NHC1^(Theta)) has pH of 2.89 . Calculate pK_(b) for pyridine (C_(5)H_(5)N) .

The percentage of pyridine (C_(5)H_(5)N) that forms pyridinium ion (C_(5)H_(5)N^(+)H) in a 0.10 M aqueous pyridine solution ( K_(b) for C_(5)H_(5)N=1.7xx10^(-9) ) is

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

Calculate the pH of 1.0 L of 0.10 M pyridine solution to which 0.3 mol of pyridinium chloride C_5H_5NH^+Cl , has been added, assuming no change in volume.

Predict the effect of addition of pyridinium ion C_5H_5NH^+ on the position of the equilibrium. Will the pH be raised or lowered ?

Determine the pH of a 0.2 M solution of pyridine C_5H_5N. K_b= 1.5 xx 10^(-9)

MOTION-IONIC EQUILIBRUIM-Exercise -3
  1. What is the OH^(-) concentration of a 0.08 M solution of [K(a)(CH(3)CO...

    Text Solution

    |

  2. Calculate the pH of a 2.0 M solution of NH4Cl. [Kb(NH3)= 1.8 xx 10^(-5...

    Text Solution

    |

  3. A 0.25 M solution of pyridinium chloride C(5)H(5)NH^(+)Cl^(-) was foun...

    Text Solution

    |

  4. Calculate the extent of hydrolysis & the pH of 0.02 M CH3COONH4. [K(...

    Text Solution

    |

  5. Calculate the percent hydrolysis in a 0.06 M solution of KCN. [Ka(HCN)...

    Text Solution

    |

  6. Calculate the extent of hydrolysis of 0.005 M K2CrO4. [K2= 3.1 xx 10^(...

    Text Solution

    |

  7. Calculate the percent hydrolysis in a 0.0100 M solution of KCN. (Ka= 6...

    Text Solution

    |

  8. A 0.010 M solution of PuO2(NO3)2 was found to have a pH of 4.0. What i...

    Text Solution

    |

  9. At what pH will a 1.0 xx 10^(-3)M solution of an indicator with K(b) =...

    Text Solution

    |

  10. Calculate the pH of 0.010M NaHCO(3) solution. K(1)=4.5xx10^(-7) , K(...

    Text Solution

    |

  11. Calculate the pH of 0.05 M KHC(8)H(4)O(4) H(2)C(8)H(4)O(4) + H(2)O ...

    Text Solution

    |

  12. The acid ionization (hydrolysis) constant of Zn^(2+)" is "1.0 xx 10^(-...

    Text Solution

    |

  13. The acid ionization (hydrolysis) constant of Zn^(2+)" is "1.0 xx 10^(-...

    Text Solution

    |

  14. Determine [overset(Θ)OH] of a 0.050M solution of ammonia to which suff...

    Text Solution

    |

  15. Calculate the pH of solution prepared by mixing 50.0 mL of 0.200 M HC2...

    Text Solution

    |

  16. A buffer of pH 9.26 is made by dissolving x moles of ammonium sulphate...

    Text Solution

    |

  17. 50 mL of 0.1 M NaOH is added to 75 mL of 0.1 M NH4Cl to make a basic b...

    Text Solution

    |

  18. Determine the pH of a 0.2 M solution of pyridine C5H5N. Kb= 1.5 xx 10^...

    Text Solution

    |

  19. Predict the effect of addition of pyridinium ion C5H5NH^+ on the posit...

    Text Solution

    |

  20. Calculate the pH of 1.0 L of 0.10 M pyridine solution to which 0.3 mol...

    Text Solution

    |